Net Ionic Equations and Spectator Ions

This video tutorial guides viewers through writing a balanced net ionic equation for the reaction between sulfuric acid (H2SO4) and sodium sulfide (Na2S). It begins with balancing the molecular equation, assigning states to each substance, and discussing the dissociation of strong electrolytes. The tutorial then demonstrates how to form the complete ionic equation by splitting strong electrolytes into ions. Spectator ions are identified and removed to derive the net ionic equation. The video concludes by ensuring charge balance and summarizing the process.

What is the first step in balancing net ionic equations?

• Balance the molecular equation

• Write the complete ionic equation

• Identify spectator ions

• Determine the states of substances

Which of the following is a strong electrolyte?

• H2S

• Na2S

• H2O

• CO2

What is the state of sulfuric acid in the reaction?

• Solid

• Gas

• Liquid

• Aqueous

What is the charge of the sulfate ion?

• 1+

• 2+

• 2-

• 1-

Which ion is not split in the complete ionic equation because it is a gas?

• SO4 2-

• Na+

• S 2-

• H2S

What is the role of spectator ions in a net ionic equation?

• They change the charge balance

• They are removed from the equation

• They participate in the reaction

• They form new compounds

Which ions are considered spectator ions in this reaction?

• H+ and S 2-

• Na+ and SO4 2-

• H2S and Na+

• SO4 2- and H+

What is the net charge on both sides of the balanced net ionic equation?

• 1+

• 2-

• 0

• 2+

If H2S were aqueous, what would change in the net ionic equation?

• A new compound would form

• The equation would remain the same

• H2S would be split into ions

• The charge balance would change

What ensures the net ionic equation is correctly balanced?

• Equal number of atoms on both sides

• Equal number of molecules on both sides

• Equal number of compounds on both sides

• Equal number of electrons on both sides